Question

Draw the electron dot structure of ${{\rm{F}}_{\rm{2}}}$ (fluorine).

Answer 1

Hint: We know that the structure of the molecules in terms of the valence electrons present in the valence shell of each atom in the molecule is referred to as Lewis structures or electron dot structure.

Complete step by step answer:
We know that Lewis structures are drawn for molecules containing either covalent bonds or coordinate bonds. These structures are drawn by placing the atoms in an order that less electronegative atom or the atom with the highest valency is kept in the center and more electronegative atoms surround it.
In Lewis dot structure, each atom is then provided with their valence electrons and sharing of electrons is done to complete their octet or doublet between the central and surrounding atoms. However, the remaining electrons belonging to valence shells are kept on each atom wherever applicable which are known as lone pairs.
In ${{\rm{F}}_{\rm{2}}}$ molecule, fluorine has the atomic number $9$. Its electronic configuration is ${\rm{1}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{p}}^{\rm{5}}}$. The number of valence electrons present in fluorine is $7$ which are present in ${\rm{2s}}$ and ${\rm{2p}}$ orbitals. Fluorine requires only one valence electron in order to complete its octet. Therefore, two atoms of fluorine form covalent bond with each other. In the representation of the electron dot structure of ${{\rm{F}}_{\rm{2}}}$, the valence electrons are represented by dots around each fluorine atom. So let’s draw the electron dot structure of ${{\rm{F}}_{\rm{2}}}$ which is shown below.

There is one bonded pair of electrons and three lone pairs of electrons on each fluorine atom.

Note:
The electron dot structures of molecules are very helpful in the determination of bonding and nonbonding electron pairs.